How much water is ionized in the lightning?

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The discussion centers on calculating the amount of water ionized during a lightning strike. The participant attempts to determine the mass of water ionized by using the molar mass of water (18.1 g/mol) and Avogadro's number (6.02214e23 molecules/mol). However, the calculation presented (3.005576e-23) is incorrect due to unit misalignment. The conversation highlights the need for additional information regarding the total charge in a lightning bolt to accurately assess the fraction of electrons involved in water ionization.

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  • Understanding of mole concept and molar mass
  • Familiarity with Avogadro's number
  • Basic knowledge of electrical charge and coulombs
  • Concept of ionization in chemistry
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Students in chemistry and physics, educators teaching about electrical phenomena, and anyone interested in the chemical processes involved in lightning strikes.

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If each water molecule donates one electron,
how much water is ionized in the lightning?
One mole of water has a mass of 18.1 g/mol.
Answer in units of g.


Avogadro’s number is 6.02214e23 /mol.


ok so this is what i did...
(18.1grams/1mole)(1mol/6.02214e23 molecules)=3.005576e-23
this is wrong since it doesn't give the right units. How would i do this?
 
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How many coulombs in that bolt of lightning and what fraction of those electrons are involved in the ionization of water.

Not enough information but I'm guessing the answer is 42.
 
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